3. The following reaction reaches equilibrium at 650 ˚C and atmospheric pressure: N2 (g) + C2H2 (g)  2HCN (g) If the system initially is an equimolar mixture of nitrogen and acetylene, what is the composition of the system at equilibrium? What would be the effect of doubling the pressure? Assume ideal gases.

Before giving you an answer, I want to clarify that this question is poorly written, or confusing.

Although an equimolar reaction means that it maintains the same number of molecules at the beginning and at the end of the reaction of one or two compounds.

Explanation:

Considering that it is an ideal gas, ideal gases are so named because they comply with a behavior where they maintain their number of moles and the constant r = 0.082x10exp23.

In this way we deduce that the equation that we would have to take into account is: P x V = n x r x T

where P is pressure, V is volume, n is number of moles, r is the ideal gas constant, and T is temperature.

Now, if we look at the equation, we can realize that if the pressure of this ideal gas increases, the VOLUME would decrease and the TEMPERATURE could increase.

This phenomenon of temperature occurs because the compression of the gas generates greater proximity between the molecules, and therefore greater friction between them, increasing the temperature.